A student measures the solubility of \(\text{O}_2\text{(g)}\) and \(\text{SO}_2\text{(g)}\) in pure water at \(293\text{ K}\) and a constant partial pressure of \(1.0\text{ atm}\), obtaining the data presented in the table below.

Gas	Molecular geometry	Polarity	Solubility at \(293\text{ K}\) (\(\text{mol/L}\))
\(\text{O}_2\)	Linear	Nonpolar	\(1.4 \times 10^{-3}\)
\(\text{SO}_2\)	Bent	Polar	\(1.5\)

If the temperature of both saturated aqueous solutions is raised to \(333\text{ K}\) while maintaining a constant partial pressure of \(1.0\text{ atm}\) for each gas, which of the following correctly predicts the outcome on the solubility of each gas and provides the best justification based on intermolecular forces?